Final Semester 1—Review Sheet Chapter 1&3—What is Chemistry • Matter • Mass • Weight • Scientific method o Observation § Observation vs. inference (know the difference) § Qualitative data § Quantitative data o Hypothesis o Experimentation § Dependent variable § Independent variable § Control o Data analysis o Conclusion § Scientific theory § Scientific law • Measurement • The Metric System o Standard units of measurement (SI units) § Length (m) § Mass (kg) § Temperature (K) • °C + 273 = Kelvin (K) § Time (s) § Substance (mol) o Prefixes § Kilo § Centi § Milli • Scientific notation (know how to write both big and small numbers in scientific notation) • Accuracy If I gave you a set of numbers could you tell if they were accurate, precise, neither, or both • Precision • Percent error (know how to calculate) • Significant figures o Know how to find sig. figs § With a decimal § Without a decimal § Numbers in scientific notation o Rounding numbers with sig. figs. o Adding and subtracting numbers with sig. figs o Multiplying and dividing numbers with sig. figs • Density •
o Equation D=m/v o Know different units § Liquid g/mL § Solid g/cm3 § Gas: g/L o Properties o Word problems with density!! Dimensional analysis Chapter 2—Matter • Properties of matter o Physical property Be able to provide examples o Chemical property • Substance • Extensive • Intensive • States of matter • Changes in matter o Physical change Be able to provide examples o Chemical change • Reactant • Product • Law of conservation of mass • Signs of a chemical reaction • Mixture o Homogeneous § Alloy § Solution o Heterogeneous • How to separate mixtures o Crystallization o Distillation o Filtration o Chromatography • Element (identify the following on the periodic table for any given element) o Symbol o Atomic mass o Atomic number o Name • Compound Chapter 4 & 25—Nuclear Chemistry • Atom • Dalton’s Atomic Theory • Subatomic particle o Proton o Neutron o Electron • J.J. Thompson’s Plumb Pudding Model • Rutherford’s Gold Foil Experiment •
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o What he used o What he thought would happen o What actually happened o His conclusion The nuclear atom Atomic number (equal to # of protons) Mass number (sum of protons and neutrons) Isotope (same atom different number of neutrons) Atomic mass o Unit for atomic mass is amu (atomic mass unit) o Know how we derived the amu!! o Weighted average Radioactivity Radioactive decay o Why does an atom undergo radioactive decay? (to become stable) Types of radiation o Alpha radiation § Alpha particle (helium nucleus)!! KNOW SYMBOL § Stopped by paper § Least penetrating o Beta radiation § Beta particle (electron) KNOW SYMBOL § Stopped by metal foil or wood o Gama radiation § Gamma particle (pure energy) KNOW SYMBOL § Not completely blocked by lead or concrete § Most penetrating Electrostatic force o Electrostatic repulsion (like charges) o Electrostatic attraction (opposite charges) Strong nuclear force (keeps the nucleus of an atom together)!! Know how to write and balance nuclear equations!! Transmutation Half-­‐life Nuclear fusion Nuclear fission Energy released in a nuclear reaction is much greater than that in a chemical reaction!! Mass defect Chapter 5 & 6—Energy, Models of the Atom, and The Periodic Table • Electromagnetic radiation • Electromagnetic spectrum • Wavelength Inversely proportional!! • Frequency • Energy • Visible light (think of the rainbow) o Red—longest wavelength, lowest frequency o Violet—shortest wavelength, highest frequency • Photon • Excited state •
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Ground state Atomic spectra o Emission o Absorption o Continuous Bohr Model of the atom Quantum mechanical model of the atom Atomic orbital Quantum numbers o Principal quantum number (1-­‐7; corresponds to the period an element is in) o Energy sublevel (s, p, d, f ; corresponds the shape where an electron could be found) § Know the s, p, d, f blocks of the periodic table!! o Atomic orbital (corresponds to an electrons location) § s sublevel has 1 orbital (2 electrons total) § p sublevel has 3 orbital (6 electrons total) § d sublevel has 5 orbital (10 electrons total ) § f sublevel has 7 orbital (14 electrons total) Electron configuration Noble gas configuration Aufbau principle Pauli Exclusion principle Hunds Rule Valence electron Lewis Dot diagram Periodic Law Periodic table (identify the following on the periodic table) o Group § Alkali metals § Alkaline earth metals § Halogens § Noble gas o Period o Metal o Nonmetal o Metalloid o Representative elements (group A) o Transition elements (group B) Properties of metals Be able to tell the difference Properties of nonmetals Periodic trends (both across a period (left to right) and down a group (top to bottom)) o Atomic radius § Shielding o Electronegativity § Most electronegative element on the periodic table? o Ionization energy Chapter 7 & 9—Ionic Compounds and Naming • Chemical bonds o Ionic o Covalent •
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o Metallic Reactivity of elements Octet Rule Ions (know the charges of group A elements on the periodic table, except 4A) o Cation § Monatomic § Polyatomic (given to you) o Anion § Monatomic § Polyatomic (given to you) Ionic compounds o Formation o Properties o Shape (crystal lattice) Formula unit (know how to write an ionic formula if given the name, and how to write the name if given a formula)!!!! Electrolyte Electron Sea Model Delocalized electron Chapter 8 & 9—Covalent Compounds and Naming • Covalent bond o Single o Double o Triple • Covalent bond strength (different for each type, think of the pencil demo) o Factors in determining strength • Covalent bond length (different for each type, think of the pencil demo)Co • Molecule • Diatomic molecules (you need to memorize these)!! o HONClBRIF o Magnificent 7 • Covalent molecules o Formation o Properties • Binary Molecular compounds (know how to write a covalent formula if given the name, and how to write the name if given a formula)!!!! • Lewis structure o Simple o Ions o Multiple bonds o Incomplete octet § Exceptions to the octet rule (HAlBBe)!! o Resonance • VSEPR theory (only know the following statement)!!!! o Used to predict shape of a molecule • Polarity (determined by difference in electronegativity or symmetry of molecules) o Ionic (biggest difference in electronegativity and the most polar molecules) o Polar covalent o Nonpolar covalent •
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Intermolecular forces o Dispersion force o Dipole-­‐Dipole o Hydrogen bond Solubility of molecules (like dissolves like)